HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr | Hoàn thành PTHH

Question: Complete the following PTH: HCOOCH3 + Br2 + FRIENDS2O → ONLY3HCO3 + HBr

Answer:

HCOOCH3 + Br2 + FRIENDS2O → ONLY3HCO3 + 2HBr

Join Trinh Hoai Duc High School to expand your knowledge of bromine!

1. What is Bromine?

– Bromine is the third chemical element of the Halogen group, with the symbol Br, is a reddish brown fuming liquid at room temperature, which evaporates easily to form a similar colored gas.

Pure bromine is very reactive, so bromine does not exist in the không lấy phí form in nature, but mainly exists in the form of colorless soluble crystalline mineral halogen salts, similar to table salt.


2. Natural state

– In nature, bromine is found mainly in the form of compounds, most of which are bromide salts of potassium, sodium or magnesium, found in seawater and lake water. Compared with chlorine and fluorine, the bromine content in nature is less.

The two stable isotopes of bromine are: Br79 (50.69%) and Br81 (49.31%).

3. Physical properties of Bromine

+ Bromine exists in liquid form and easily ignites reddish brown at room temperature to form a gas.

+ Boiling point: 332.0 K ​ (58.8 °C, ​137.8 °F).

+ Melting point: 265.8 K ​ (-7.2 °C, 19 °F).

+ Evaporation temperature: 29.96 kJ·mol−1

+ Bromine is slightly soluble in water but more soluble in organic solvents such as ethanol, benzene, gasoline, etc.

A solution of bromine in water is called bromine water.

4 . Chemical properties

a. Effect with metal

– The corresponding salt-forming product.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 2)

b. React with hydrogen

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 3)

– Activity decreases from Cl → Br → I

– The gases HBr, HI dissolve in water to form an acidic solution.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Completing high school (photo 4)

– In terms of acid strength, it gradually increases from HCl

c. The reducing property of Br2HBr

– Bromine exhibits reducing properties when encountering strong oxidizing agents (such as chlorine water, …)

Br2 + 5Cl2 + 6 HOUSES2O → 2HBrO3 (bromic acid) + 10HCl

– The reducing property of HBr (in the gaseous state as well as in dd) is stronger than HCl. HBr can reduce H2SO4 condensed into SO2.

2HBr + HELL2SO4 dong → Br2 + SO2 + 2 HOUSES2O

– Dd HBr is colorless, left in air for a long time, becomes yellow-brown because of oxidation (dd HF and HCl do not have this reaction):

4HBr + O2 → 2 family2O + 2Br2

5. What is the application of Bromine?

+ Widely used in pharmaceuticals, in the production of dyes or inks, and in photography to make coatings

+ Used as a flame retardant with the ability to prevent or retard the combustion of plastics

– In agriculture: organic bromine compounds are raw materials for creating pesticides, killing insects, even rodents.

– In industry: As a petroleum additive. However, this application is gradually decreasing. Application in oil drilling: liquid bromide compounds are used as special drilling fluids for deep and high pressure wells.

In addition, it is also used to disinfect covered swimming pools with higher efficiency than some other disinfectants

*Modulation

– The main source for the preparation of bromine is sea water.

– Preparation of bromine based on the oxidation of Br . ionsthe oxidizing agent is chlorine.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 5)

6. Some Compounds of Bromide

Hydrogen bromide and bromhyric acid

+ Under normal temperature conditions, HBr is a gas, colorless, fuming in humid air and easily soluble in water.

A solution of HBr in water is called a solution of bromhyric acid. Hydrobromic acid, considered a strong acid.

The oxygen-containing compound of bromine

+ Hypobromo acid (HBrO) has poor stability, oxidation and acidity HClO.

+ Bromic acid (HBrO3).

+ Pebromic acid (HBrO4).

Similar to chlorine, in compounds with oxygen, bromine exhibits a positive oxidation number (+1, +3, +5, +7).

Posted by: Trinh Hoai Duc High School

Category: Grade 12, Chemistry 12

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HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr | Hoàn thành PTHH -

Question: Complete the following PTH: HCOOCH3 + Br2 + FRIENDS2O → ONLY3HCO3 + HBr

Answer:

HCOOCH3 + Br2 + FRIENDS2O → ONLY3HCO3 + 2HBr

Join Trinh Hoai Duc High School to expand your knowledge of bromine!

1. What is Bromine?

– Bromine is the third chemical element of the Halogen group, with the symbol Br, is a reddish brown fuming liquid at room temperature, which evaporates easily to form a similar colored gas.

Pure bromine is very reactive, so bromine does not exist in the không lấy phí form in nature, but mainly exists in the form of colorless soluble crystalline mineral halogen salts, similar to table salt.


2. Natural state

– In nature, bromine is found mainly in the form of compounds, most of which are bromide salts of potassium, sodium or magnesium, found in seawater and lake water. Compared with chlorine and fluorine, the bromine content in nature is less.

The two stable isotopes of bromine are: Br79 (50.69%) and Br81 (49.31%).

3. Physical properties of Bromine

+ Bromine exists in liquid form and easily ignites reddish brown at room temperature to form a gas.

+ Boiling point: 332.0 K ​ (58.8 °C, ​137.8 °F).

+ Melting point: 265.8 K ​ (-7.2 °C, 19 °F).

+ Evaporation temperature: 29.96 kJ·mol−1

+ Bromine is slightly soluble in water but more soluble in organic solvents such as ethanol, benzene, gasoline, etc.

A solution of bromine in water is called bromine water.

4 . Chemical properties

a. Effect with metal

- The corresponding salt-forming product.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 2)

b. React with hydrogen

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 3)

– Activity decreases from Cl → Br → I

– The gases HBr, HI dissolve in water to form an acidic solution.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Completing high school (photo 4)

– In terms of acid strength, it gradually increases from HCl

c. The reducing property of Br2HBr

- Bromine exhibits reducing properties when encountering strong oxidizing agents (such as chlorine water, ...)

Br2 + 5Cl2 + 6 HOUSES2O → 2HBrO3 (bromic acid) + 10HCl

– The reducing property of HBr (in the gaseous state as well as in dd) is stronger than HCl. HBr can reduce H2SO4 condensed into SO2.

2HBr + HELL2SO4 dong → Br2 + SO2 + 2 HOUSES2O

– Dd HBr is colorless, left in air for a long time, becomes yellow-brown because of oxidation (dd HF and HCl do not have this reaction):

4HBr + O2 → 2 family2O + 2Br2

5. What is the application of Bromine?

+ Widely used in pharmaceuticals, in the production of dyes or inks, and in photography to make coatings

+ Used as a flame retardant with the ability to prevent or retard the combustion of plastics

– In agriculture: organic bromine compounds are raw materials for creating pesticides, killing insects, even rodents.

– In industry: As a petroleum additive. However, this application is gradually decreasing. Application in oil drilling: liquid bromide compounds are used as special drilling fluids for deep and high pressure wells.

In addition, it is also used to disinfect covered swimming pools with higher efficiency than some other disinfectants

*Modulation

– The main source for the preparation of bromine is sea water.

- Preparation of bromine based on the oxidation of Br . ionsthe oxidizing agent is chlorine.

HCOOCH3 + Br2 + H2O → CH3HCO3 + HBr |  Complete high school (photo 5)

6. Some Compounds of Bromide

Hydrogen bromide and bromhyric acid

+ Under normal temperature conditions, HBr is a gas, colorless, fuming in humid air and easily soluble in water.

A solution of HBr in water is called a solution of bromhyric acid. Hydrobromic acid, considered a strong acid.

The oxygen-containing compound of bromine

+ Hypobromo acid (HBrO) has poor stability, oxidation and acidity HClO.

+ Bromic acid (HBrO3).

+ Pebromic acid (HBrO4).

Similar to chlorine, in compounds with oxygen, bromine exhibits a positive oxidation number (+1, +3, +5, +7).

Posted by: Trinh Hoai Duc High School

Category: Grade 12, Chemistry 12

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